Unit 2
Types of Chemical Reactions
Problem Set
18. A 0.0500 M solution of potassium permanganate was used to titrate 250.0 mL of a platinum (II)
chloride solution with an unknown concentration. The endpoint was reached after 26.87 mL of
0.0500 M KMnO4 were delivered.
a.
Write the balanced net ionic equation for the chemical reaction that occurred during this
titration.
b. How many moles of KMnO4 were delivered when the endpoint was reached?
c. How many moles of platinum chloride were contained in the 250.0 mL sample?
d. Calculate the experimentally determined molar concentration (M) of platinum (II) chloride in
solution.
Unit 2
Types of Chemical Reactions
Problem Set
19. In a gravimetric experiment 200. mL of 2.0 M copper (I) nitrate is mixed with 150. mL of 2.5 M
sodium chloride. The mixture produces a precipitate.
a. Identify the precipitate
b. What is the limiting reactant? Justify your answer
c. What is the maximum mass of precipitate that can be formed in this reaction?
d. What is the percent yield if 31 g of precipitate is formed in the reaction?
e. The percentage yield increases when the temperature of the solution is reduced. Explain why
this is.
Unit 2
Types of Chemical Reactions
Problem Set
20. A gravimetric experiment was performed to determine the number of moles of sulfate that were
present in a solution of sodium sulfate. In this experiment, an excess of barium nitrate was added to
the solution and a precipitate formed. The resulting mixture was filtered and the precipitate was
dried. The dry mass of the precipitate was measure to be 8.642 g.
a. Write the balanced complete ionic equation for the precipitation reaction
b. Write balanced net ionic equation for the precipitation reaction.
c.
Calculate the number of moles of sulfate in the sample.